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Henry's Law
- c = kP
- solubility (in mol/L) = Henry's law constant (in mol/L·atm) x partial pressure (atm)
- it's a law stating the concentration of a gas in a solution is proportional to the pressure of that gas over the solution
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colloid
stable but non-homogenous mixtures; an intermediate between a stable solution and unstable heterogeneous mixtures
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hard water
water that has high mineral content, such as Ca2+ and Mg2+ ions
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ion exchange
an exchange of ions between two electrolytes or between an electrolyte solution and a complex
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amino acid
monomers of proteins; organic compounds composed of an amine and carboxyl groups in the same molecule
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random coil
a polymer conformation where the monomer subunits are oriented randomly while still being bonded to adjacent units. It is not one specific shape, but a statistical distribution of shapes for all the chains in a population of macromolecules
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mononucelotide
monomers of nucleic acids; consists of an N-containing base, a sugar, and a phosphate group
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crystal defect
periods of interruption in the regular pattern of a crystalline solid's exhibit periodic crystal structure
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phase
a physically distinctive form of matter, such as a solid, liquid, gas; it is generally characterized by having relatively uniform chemical and physical properties
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crosslink
ionic or covalent bonds that link one polymer chain to another
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doping
the practice of adding impurities to something
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plastic
polymers of high molecular mass; made up of monomers that are organic compounds (are either natural or synthetic)
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ceramic
an inorganic, nonmetallic solid prepared by the action of heat and subsequent cooling; such materials may have a crystalline or amorphous structure (e.g. glass)
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soap
the salt of a strong base (metal hydroxide) and a fatty acid (aka a carboxylic acid with a long hydrocarbon chain)
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in a saturated solution, there is a dynamic equillibrium between the solid phase and the solvated phase; the solid phase __________ at the same rate as the solvated phase ___________
dissolves; crystalizes
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through the influence of intermolecular forces among the protein's side chains, soluble proteins have __________ exteriors, and ________ interiors
polar-ionic exteriors, and nonpolar interiors
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solvation
the process of surrounding a solute particle with solvent particles; solvation in water is called hydration
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Molarity (M)
- mol of solute/volume (L) of solution
- because volume is affected by temperature, MOLARITY IS AFFECTED BY TEMPERATURE
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molality (m)
- mol of solute/mass of solvent (in kg)
- better for problems where temperature or density (volume) change B/C it's temperature independent (used in BP/FB problems)
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boiling point
the temperature at which its vapor pressure equals the external pressure; the addition of a solute LOWERS the vapor pressure so it has to be heated to a HIGHER temperature in order to boil
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the boiling point of a solution (Tb) is always _______ than the boiling point of the pure solvent (Tb0)
HIGHER
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boiling point of a solution
- ΔTb = Kbm
- boiling point = molal boiling point elevation CONSTANT x molality (mol solute/kg solvent)
- ΔTb=Tb - Tb0 (aka boiling point = boiling point of the soution minus the boiling point of the solvent)
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the addition of a solute to a liquid (solvent) will ______ the FREEZING point
LOWER (oppsite of b.p.); think lowering is why you put the negative sign in front
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freezing point of a solution
- ΔTf = -Kfm
- freezing point = - molal freezing point elevation CONSTANT (for solvent only) x molality (mol solute/kg solvent)
- ΔTf=Tf - Tf0 (aka freezing point = freezing point of the soution minus the freezing point of the solvent)
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osmosis
the tendency for solvent to flow from areas of low concentration to areas of high concentration (this time concentration means the concentration of solute, so if there's more solute on one side than another the solvent will GO to that side to try to 'dilute' it almost)
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osmotic pressure
the amount of pressure necessary to stop osmosis (essentially the strong/maximal pressure exerted on the semi-permeable membrane by the side with more volume [the side where a lot of solvent dissolved into because it had a high concentration of solute]); it can be simulated by us!
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magnitude of osmotic pressure =
- π
- π = MRT which means...
- osmot. pressure = (molarity of the solution)(funky gas constant)(temperature in Kelvin)
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Crenation
the contraction of a cell after exposure to a hypertonic solution, due to the loss of water through osmosis
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Hemolysis
when water flows into a cell causing it to swell/burst because the solute concentration inside the cell is higher meaning the osmotic pressure of the intracellular fluid of a red blood cell is hIGHER than that of the solution surrounding the cell
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colligative properties
properties that depend on the concentration of solute particles NOT the identity of the solute particles
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electrolytes
substances that dissociate into ions when dissolved (solution will conduct electrical current)
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van't Hoff factor (i)
- used to modify the colligative property expressions to reflect the (possible) dissociation of a solute; inserted in to the colligative property expressions (BP, FP, and osmotic pressure)
- i = # ions in solutions / # formula units in solution
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the van't Hoff factor should be an integer for a ______ electrolyte:
strong electrolyte; this is because a strong electrolyte is supposed to dissociate completely
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Brownian motion
the random drifting of particles suspended in a fluid (liquid or gas)
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Tyndall effect
when a beam of light passes through a colloid the beam of light is visible when viewed perpendicularly; if a beam of light passes through a true solution, it isn't visible from that perspective
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flocculation
a process where colloids come out of suspension in the form of floc or flakes due to a change in concentration of ions or the introduction of ions in the dispersion
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